A student produced a soluble salt by reacting nickel carbonate with dilute nitric acid.
This is the method used:
Complete the word equation for the reaction. nickel carbonate+nitric acid→‾+‾+carbon dioxide\text{nickel carbonate} + \text{nitric acid} \rightarrow \text{\underline{\quad\quad\quad\quad\quad\quad}} + \text{\underline{\quad\quad\quad\quad\quad\quad}} + \text{carbon dioxide}nickel carbonate+nitric acid→++carbon dioxide
Give one observation the student could make during Step 4 which shows that the nickel carbonate is in excess.
Give one reason for filtering the mixture in Step 5.
Name the equipment that can be used to warm the filtrate gently in Step 6.
The maximum theoretical mass of the nickel nitrate crystals that could be produced is 14.50 g14.50\text{ g}14.50 g. The percentage yield of the crystals is 82.0%82.0\%82.0%.
Calculate the mass of crystals actually produced. Use the equation: Percentage yield=mass of salt actually producedmaximum theoretical mass of salt×100\text{Percentage yield} = \frac{\text{mass of salt actually produced}}{\text{maximum theoretical mass of salt}} \times 100Percentage yield=maximum theoretical mass of saltmass of salt actually produced×100